The following steps will guide you through balancing redox reactions -

1. Balance elements in the equation other than O and H.

2. Balance the oxygen atoms by adding the appropriate number of water (H₂O) molecules to the opposite side of the equation.

3. Balance the hydrogen atoms (including those added in step 2 to balance the oxygen atom) by adding H⁺ ions to the opposite side of the equation.              

4. Add up the charges on each side. Make them equal by adding enough electrons (e^-) to the more positive side. (Rule of thumb: e^- and H⁺ are almost always on the same side).

5. The e^- on each side must be made equal; if they are not equal, they must be multiplied by appropriate integers (the lowest common multiple) to be made the same.

6. The half-equations are added together, canceling out the electrons to form one balanced equation. Common terms should also be canceled out.